For the electrode reaction, Mn+(aq)+ne- xrightarrow[]M(s) Nernst equation is

Question

For the electrode reaction, Mn+(aq)+ne- xrightarrow[]M(s) Nernst equation is (A)  E=E° +(RT/nF) log (1/[Mn+])  (B)  E° =E+RT in [Mn+]  (C)  E=E° -(RT/nF) in(1/ [Mn+])  (D)  (E/E° )=(RT/nF) in[Mn+]

Tardigrade Admin · Accepted Answer

For the electron reaction, Mn+(aq)+ne- xrightarrow[]M(s) Nernst equation is E=E° -(RT/nF)in(1/[Mn+])

Q. For the electrode reaction, $M^{n +} (a q) + n e^{-} M (s)$ Nernst equation is

$E = E^{\circ} + \frac{RT}{n F} lo g \frac{1}{[ M ^{n +} ]}$

$E^{\circ} = E + RT in [M^{n +}]$

$E = E^{\circ} - \frac{RT}{n F} in \frac{1}{[ M ^{n +} ]}$

$\frac{E}{E ^{\circ}} = \frac{RT}{n F} in [M^{n +}]$

For the electron reaction, $M^{n +} (a q) + n e^{-} M (s)$ Nernst equation is $E = E^{\circ} - \frac{RT}{n F} in \frac{1}{[ M ^{n +} ]}$

Q. For the electrode reaction, Mn+(aq)+ne−​M(s) Nernst equation is

E=E∘+nFRT​log[Mn+]1​

E∘=E+RTin[Mn+]

E=E∘−nFRT​in[Mn+]1​

E∘E​=nFRT​in[Mn+]